Homework Help: chem/solubility

Posted by Natash on Wednesday, May 13, 2009 at 11:31pm.

the Ksp of CaF2 = 1.46*10^-10 and Ka of HF = 3.5*10^-4 Calculate the pH of a solution in which the solubility of CaF2 = .0100 moles/liter.

so Ksp =[Ca2+][F-]^2 and
Ka =[H3O+][F-]/[HF]

I'm not sure how to continue...

chem/solubility - DrBob222, Thursday, May 14, 2009 at 1:07am
You need another equation.
2*solubility = (F^-) + (HF)
That + Ksp + Ka
Solve for (H^+).
I get 0.0579 M = (H^+) or pH of 1.237 which rounds to pH = 1.24.
Using 1.24 and going through it from the front end give S = 0.0100. I hope this helps.

Answer this Question

Related Questions

chemistry - Given a saturated solution of CaF2, write the ionic equilibrium and ...
Chemistry - What is the molar solubility of CaF2 if o,1o mol of NaF are added to...
Chemistry - Given a saturated solution of CaF2, write the ionic equilibrium and ...
Chemistry 114 - Write down the Ksp expression for CaF2. If the molar solubility ...
chem - The molar solubility of MgF2 at 25°C is 1.2 10-3 mol/L. Calculate ...
chemistry - The mineral CaF2 has a solubility of 2.1 x 10^-4 M. What is the Ksp ...
chemistry - the Ksp for CaF2 is 3.9*10-11. assuming that calcium flouride ...
Chemistry - At saturation 1.5 x 10^-4 moles caF2 have dissolved in 1L of water. ...
Chem - (a) The molar solubility of Ag2CrO4(s) at 35°C is 1.3 10-4 mol/L. ...
Chemistry - Consider a saturated solution of calcium fluoride in 0.086 M ...

For Further Reading

First Name:
School Subject:
Answer: